The vapor density of a gas is $11.2$. At $N.T.P.$,$11.2 \ g$ of this gas occupies a volume of ............. $litres$.

If the density of air at $STP$ is $0.001293 \, g \, mL^{-1}$,what will be its vapor density?

Which of the following equations is correct for the vapour density of completely dissociated ammonium chloride?

Phosphorus pentachloride dissociates as follows,in a closed reaction vessel:
$PCl_{5(g)} \rightleftharpoons PCl_{3(g)} + Cl_{2(g)}$
If total pressure at equilibrium of the reaction mixture is $P$ and degree of dissociation of $PCl_5$ is $x,$ the partial pressure of $PCl_3$ will be:

In a $Victor \ Meyer$ experiment,$0.23 \ g$ of a volatile substance displaces $112 \ mL$ of air at $STP$. Calculate the vapor density of the substance.

The vapour density of undecomposed $N_2O_4$ is $46$. When heated,the vapour density decreases to $24.5$ due to its dissociation into $NO_{2(g)}$. The percentage dissociation of $N_2O_4$ is: